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CBSE Questions for Class 11 Medical Chemistry Some Basic Concepts Of Chemistry Quiz 9 - MCQExams.com

What mass of NaCl would contain the same total number of ions as 245 g of MgCl2?
  • 245 g
  • 225 g
  • 263 g
  • None of these
AgNO3 sample is 85% by mass. To prepare 12.5 m of 0.05 molar AgNO3 solution, AgNO3 sample  required is:
  • 2.36 g
  • 1.25 g
  • 1.49 g
  • none of these
A fresh H2O2 solution is labeled as 11.2V. Calculate its concentration in wt/vol percent.
  • 3.03
  • 6.8
  • 1.7
  • 13.6
According to the CaCO3+HClCaCl2+CO2+H2O. What mass of CaCO3 is required to react completely with 25ml. of 0.75M HCl?
  • 0.9945 g
  • 0.6645 g
  • 0.9375 g
  • 0.8555 g
Two flasks A and B of 500 mL each are respectively filled with O2 and SO2 at 300K and 1 atm pressure. The flasks contain:
  • the same number of atoms
  • the same number of molecules
  • more number of moles in flask A as compared to flask B
  • the same mass of gases
15 g of methyl alcohol is present in 100 mL of solution. If the density of solution is 0.96 g mL1, Calculate the mass percentage of methyl alcohol in solution.
  • 45.23%
  • 15.66%
  • 25.36%
  • None of these
A gas cylinder was found unattended in a public place. The investigating team took the collected samples from it. The density of the gas was found to be 2.380 gL1 at 15oC and pressure. Hence the molar mass of the gas is:
  • 30
  • 71
  • 32
  • 58
What is the mass of the precipitate formed when 50mL of 16.9% solution of AgNO3 is mixed with 
50 mL of 5.8% NaCl solution ?
(Ag = 107.8, N =14, O = 16, Na = 23, Cl=35.5)
  • 7 g
  • 14 g
  • 28 g
  • 3.5 g
Pehal and Ishaan were making 100g sugar solution with concentration by mass 20% and 50% respectively. Pehal added 20g of sugar in her solution whereas ishaan evaporated 20g of water from his solution. Now, the solutions were mixed to form a final solution, The concentration by mass of final solution is:
  • 28%
  • 45%
  • 40%
  • 60%
3.49g of ammonia at STP occupies a volume of 4.48 dm3 calculate the molar mass of ammonia. 
  • 13.25 g/mol
  • 14.59 g/mol
  • 17.45 g/mol
  • None of these
Two isotopes of an elements Q are Q97 (23.4% abundance) and Q94 (76.6% abundance). Q97 is 8.082 times heavier than C12  and Q94 is 7.833 times heavier than is C12. What is the average atomic weight of the elements Q?
  • 94.702
  • 78.913
  • 96.298
  • 94.695
1 g-atom of nitrogen atom represents:
  • 6.02×1023 N2 molecules 
  • 22.4 L of N2 at S.T.P
  • 11.2 L of N2 at S.T.P.
  • 28g of nitrogen
A solution of ethanol in water is 10% by volume. If the solution and pure ethanol have densities of 0.9866 g/cc and 0.785 g/cc respectively. The percent by weight is nearly?
  • 7.95%
  • 17%
  • 9.86%
  • 16.2%
10g of glucose is dissolved in 150g of water. The mass percantage of glucose is:
  • 2.50%
  • 6.67%
  • 8.75%
  • 10%
N2 gas is present in one litre flask at a pressure of 7.6×1010 mm of Hg. The number of N2 gas molecules in the flask at OoC is?
  • 2.68×109
  • 2.68×1010
  • 1.34×1028
  • 2.68×1022
If one gram of S contains x atoms, atoms is one gram O will be:
  • x
  • x/2
  • 23x
  • 2x
In a test tube, there is 18 g of glucose (C6H12O6)0.08 mole of glucose is taken out. Glucose left in the test tube is:
  • 0.10 g
  • 0.02 g
  • 0.10 mole
  • 3.60 g
Rearrange the following in the order of increasing mass and choose the correct order (Atomic mass, N=14,O=16,Cu=63)
(I) 1 molecule of oxygen
(2) 1 atom of nitrogen
(3) 1×1010gm molecule of oxygen
(4) 1×1010gm of copper
  • II<I<IV<III
  • IV<III<II<I
  • II<III<I<IV
  • III<IV<I<II
The number of g molecule of oxygen in 6.0×1024 molecules of CO gas is:
  • 1g molecule
  • 0.5g molecule
  • 5g molecule
  • 10g molecule
1.5gm mixture of SiO2 and Fe2O3 on very strong heating leave a residue weighting 1.46gm. The reaction responsible for loss of weight is
Fe2O3(s)Fe3O4(s)+O2(g)
What is the percentage by mass of Fe2O3 in original sample?
  • 80%
  • 20%
  • 40%
  • 60%
Calculate number of electrons present in 9.5 g of PO34.
  • 6 NA
  • 4.7 NA
  • 5 NA
  • 0.1 NA
The density of a 3M sodium thiosulphate (Na2S2O3) solution is 1.25gm/ml. Calculate the percentage by weight of sodium thiosulphate.
  • 73.92
  • 65.84
  • 17.14
  • 37.92
The mass of 50%(w/w) solution of HCl required to react with 100 g of CaCO3 would be?
  • 73 g
  • 100 g
  • 146 g
  • 200 g
Equivalent wt.of a metal is 2.5 times higher than oxygen. The ratio of weight of metal to the oxide is:
  • 0.4
  • 1.4
  • 2.4
  • 3.4
"One gram moecule of gas at N.T.P occupies 22.4 litres." This fact was derived from?
  • Dalton's therory
  • Avogadro's hypothesis
  • Berzelius hypothesis
  • Law of gaseous volume
One mole of a mixture of CO and CO2 requires exactly 20 g of NaOH in solution for complete conversion of all the CO2 into Na2CO3. How much NaOH would it require for conversion into Na2CO3, if the mixture (one mole) is completely oxidized to CO2?
  • 60 g
  • 80 g
  • 40 g
  • 20 g
Vapour density of the equilibrium mixture of NO2 and N2O4 is found to be 40 for the equilibrium: 

N2O42NO2

Calculate the percentage of NO2 in the mixture?
  • 10%
  • 5%
  • 26.08%
  • None of these
An unknown  chlorohydrocarbon as 3.55% of chlorine. If each molecule of the hydrocarbon has one chlorine atom only, chlorine atoms present in 1g of chlorohydrocarbon are: (Atomic wt. of Cl=35.5u; Avogadro constant=6.023×1023mol1)
  • 6.032×109
  • 6.032×1023
  • 6.032×1021
  • 6.032×1020
400mg capsule contains 100mg of ferrous fumarate. The percentage of iron present in the capsule approximately is: (Mol mass of Fe(C4H2O4)=170)
  • 8.2%
  • 25%
  • 16%
  • 50%
Phosphoric acid is widely used in carbonated beverages, detergents, toothpaste and fertilizers. The mass percentages of H, P and O in phosphoric acid are H3.06P31.63%,O65.31%. The atomic masses H=1,P=31 and O=16.
  • True
  • False
1g of a sample of brass om reacting with excess HCI produces 120ml of H2 gas at STP. The percentage Zn in this sample of brass is: (At.wt.of Zn-=65.5g)
  • 32%
  • 35%
  • 38%
  • 40%
In 500 grams of water dissolved 2 moles of potassium sulphate the mass precentage of salt in soluton:
  • 41%
  • 60%
  • 35%
  • 48%
The mass percentage composition of the elements in nitric acid are H=1.59%, N=22.22%, O=76.19% respectively.
(H=1,N=14,O=16)
  • True
  • False
Calculate the mass of iron which will be converted into its oxide (Fe3O4) by the action of 8g of steam on it. [At mass of Fe=56]
Fe+H2OFe3O4+4H2
  • 21g
  • 12g
  • 42g
  • 84g
What is the mass of the precipitate formed when 50 mL of 16.9 % (w/v) solution of AgNO3 is mixed with 50 mL of 5.8% (w/v) NaCl solution? 

(Ag=107.8,N=14,O=16,Na=23,Cl=35.5)
  • 7
  • 14
  • 28
  • 3.5
A solution of phosphoric acid was made by dissolving 10.0 g H3PO4
 in 100.0 mL water. The resulting volume was 104 mL. What is the , mole fraction of the solution 
  • 1
  • 2
  • 0.01
  • 3
  • 1.5
At 0C the density of gaseous oxide at 2 bar is same as that of nitrogen at 5 bar and 0C. The molar mass of the oxide is (assuming ideal behaviour): 
  • 70g/mol
  • 140g/mol
  • 28g/mol
  • 60g/mol
Calculate the mass percent of carbon in C2H5OH (Molar mass of ethanol=46.068g)
  • 13.13%
  • 88.79%
  • 52.14%
  • 34.73%
Four one litre flasks are separately filled with gases O2,F2,CH4 and CO2 under same conditions. 

The ratio of the number of molecules in these gases are:
  • 2:2:4:3
  • 1:1:1:1
  • 1:2:3:4
  • 2:2:3:4
According to Avogadro's law the volume of a gas will ____ as _____ if ____ are held constant.
  • increases, number of moles; P & T
  • decreases, number of moles; P & T
  • increases; T & P; number of moles
  • decreases; P & T; number of moles
A 1.50 g sample of an ore containing silver was dissolved,and all the Ag+ was converted to 0.125 g Ag2S. What was the percentage of silver in the ore?
  • 14.23%
  • 8.27%
  • 10.8%
  • 7.2%
To convert molality into which of the following unit of concentration require density of the solution?
  • Percentage weight by weight
  • Percentage by volume
  • Mole fraction
  • Given all
The percentage by weight of:
a] C in carbon dioxide
b] Na in sodium carbonate
c] AI in aluminium nitride.
are 27%, 43.4%, 65.85% respectively
[C=12, O=16, H=1,Na=23, AI=27, N=14]
  • True
  • False
A gaseous mixture contains CH4 and C2H6 in equimolecular proportion. The weight of 2.27 litres of this mixture at STP is:
  • 3 g
  • 4.6 g
  • 1.6 g
  • 2.3 g
25.5g of H2O2 solution on decomposition gave 1.68L of O2 at STP. The percentage strength by weight of the solution is:
  • 30
  • 10
  • 20
  • 25
100gm of an aq. solution of sugar contains 40% sugar by mass. How much water should be evaporated get 50% sugar solution by mass?
  • 10g
  • 20g
  • 0.0g
  • 40g
According to percentage weight arrange the following in descending order in the earth crust ?
  • O2,Ca,Mg,S
  • O2,S,Mg,Ca
  • S,Ca,Mg,O2
  • Ca,O2,Mg,S
One mole sample of FeO is heated in air until it is completely converted into Fe2O3. The percentage increase in weight of the sample is?
[Given: Atomic mass of Fe = 56]
  • 10.58%
  • 20.28%
  • 35.35%
  • 11.11%
Aqueous urea solution is 20% by mass of solution. Calculate percentage by mass of solvent.
  • 75%
  • 15%
  • 25%
  • 65%
The percentage weight by weight of 0.5M CCl4 solution in benzene is?
(Density of solution = 1.4g/ml)
  • 5.5%
  • 8.25%
  • 13%
  • 20.06%
0:0:2


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Practice Class 11 Medical Chemistry Quiz Questions and Answers